Related Experiment Video
Updated: Jul 8, 2026
16:11
Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
Published on: June 8, 2022
A novel two-dimensional zinc(II) coordination polymer with 6-mercaptonicotinic acid
Yong Wang1, Dong-Xia Zhu, Zhong-Min Su
1Institute of Functional Material Chemistry, Department of Chemistry, Northeast Normal University, Changchun 130024, People's Republic of China.
Acta Crystallographica. Section C, Crystal Structure Communications
|January 25, 2008
Summary
This study introduces a novel zinc(II) coordination polymer. The structure features a 2D network formed by 6-mercaptonicotinate ligands bridging zinc centers, creating a unique wavelike architecture.
Area of Science:
- Materials Science
- Inorganic Chemistry
- Crystallography
Background:
- Coordination polymers are materials with diverse applications.
- Understanding the structure-property relationships of novel coordination polymers is crucial for materials development.
Purpose of the Study:
- To synthesize and characterize a new zinc(II) coordination polymer.
- To elucidate the structural features and coordination behavior of the 6-mercaptonicotinate ligand in a zinc(II) framework.
Main Methods:
- Single-crystal X-ray diffraction was employed to determine the crystal structure.
- Analysis of coordination environments and ligand-metal interactions.
Main Results:
- A novel 2D coordination polymer, [Zn(C6H4NO2S)2]n, was successfully synthesized.
- The structure consists of two independent Zn(II) centers coordinated by 6-mercaptonicotinate (Hmna-) ligands, forming a (4,4)-network.
- The 6-mercaptonicotinate ligand acts as a bridging bidentate ligand, coordinating via sulfur and carboxyl oxygen atoms.
Conclusions:
- The coordination mode of the sulfur atoms and hydrogen bonding interactions contribute to the wavelike structure.
- This study expands the library of zinc-based coordination polymers with potential for further investigation.
Related Concept Videos
02:57Coordination Number and Geometry
For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
02:42Valence Bond Theory
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
02:34Structural Isomerism
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can be...
02:54Coordination Compounds and Nomenclature
In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
02:51Metal-Ligand Bonds
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
02:46Crystal Field Theory - Tetrahedral and Square Planar Complexes
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...